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Ionic Bonding 2008

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Ionic Bonding 2008

  1. 1. Chemical Bonds: Ionic Bonding Parts 4.2 & 4.3
  2. 2. Goal 1 Understand the basis of and describe the characteristics of ionic bonding
  3. 3. <ul><li>Why bond? </li></ul><ul><ul><li>Full outer shell </li></ul></ul><ul><ul><li>Valence electrons </li></ul></ul>
  4. 4. <ul><li>Full outer shell </li></ul><ul><ul><li>H  2 e- </li></ul></ul><ul><ul><li>All others  8 e- </li></ul></ul><ul><ul><li>Happy! </li></ul></ul>
  5. 5. <ul><li>Recall Ion formation </li></ul><ul><ul><li>Gain or loss of electron </li></ul></ul><ul><ul><li>Gain electron = “-” charge </li></ul></ul><ul><ul><li>Lose electron = “+” charge </li></ul></ul>
  6. 6. <ul><li>Characteristics of Ionic Bonds </li></ul><ul><ul><li>Metal bonded with nonmetal </li></ul></ul>
  7. 7. <ul><ul><li>Forms “ionic compounds” aka “salts” </li></ul></ul>
  8. 8. <ul><ul><li>** TRANSFER ** electrons </li></ul></ul><ul><ul><ul><li>Metals Give (+ charge) </li></ul></ul></ul><ul><ul><ul><li>Non-metals Receive (- charge) </li></ul></ul></ul>
  9. 9. <ul><ul><li>Conducts electricity only </li></ul></ul><ul><ul><ul><li>In solution </li></ul></ul></ul><ul><ul><ul><li>As liquid </li></ul></ul></ul><ul><ul><li>Because of electron movement </li></ul></ul>
  10. 10. Goal 2 Determine the chemical formula of an ionic compound by using the charge on each ion
  11. 11. <ul><li>Metals give away electrons (+ charge) </li></ul><ul><ul><li>Recall how to determine charge… </li></ul></ul><ul><ul><li>Group # </li></ul></ul><ul><ul><li>Energy levels </li></ul></ul><ul><ul><li>Li  1+ </li></ul></ul><ul><ul><li>Mg  2+ </li></ul></ul><ul><ul><li>Ca  ___ </li></ul></ul><ul><ul><li>K  ___ </li></ul></ul>
  12. 12. <ul><li>Nonmetals receive electrons ( - charge) </li></ul><ul><ul><li>Recall how to determine charge </li></ul></ul><ul><ul><li>8 electrons </li></ul></ul><ul><ul><li>Group # </li></ul></ul><ul><ul><li>Energy level </li></ul></ul><ul><ul><li>F  1- </li></ul></ul><ul><ul><li>O  2- </li></ul></ul><ul><ul><li>P  ___ </li></ul></ul><ul><ul><li>Br  ___ </li></ul></ul>
  13. 13. <ul><li>Ionic compounds strive for combined neutral (0) charge </li></ul><ul><ul><li>Neutral charge = 0 charge </li></ul></ul><ul><ul><li>Combined ions = 0 charge </li></ul></ul><ul><ul><li>Sum of charges must = 0 </li></ul></ul>
  14. 14. <ul><li>Try it… </li></ul><ul><ul><li>Na  1+ </li></ul></ul><ul><ul><li>Cl  1- </li></ul></ul><ul><ul><li>How many of each to = 0 charge? </li></ul></ul>
  15. 15. <ul><ul><li>Na 1+ and Cl 1- = 0 charge </li></ul></ul><ul><ul><li>(The charges should add to 0) </li></ul></ul><ul><ul><li>One sodium ion + One chlorine ion = 0 charge </li></ul></ul><ul><ul><li>Chemical formula is </li></ul></ul><ul><ul><li>NaCl </li></ul></ul>
  16. 16. <ul><li>That was fun! </li></ul><ul><li>Let’s try it again!! </li></ul>
  17. 17. <ul><ul><li>Mg  2+ </li></ul></ul><ul><ul><li>Cl  1- </li></ul></ul><ul><ul><li>How many of each to = 0 charge? </li></ul></ul>
  18. 18. <ul><ul><li>Mg 2+ and Cl 1- = 1+ charge </li></ul></ul><ul><ul><li>(2) + (-1) = 1 </li></ul></ul><ul><ul><li>Uh Oh!!! </li></ul></ul><ul><ul><li>One Magnesium ion + One chlorine ion = 1+ </li></ul></ul>
  19. 19. <ul><ul><li>Mg 2+ and Cl 1- and Cl 1- = 0 charge </li></ul></ul><ul><ul><li>2 + (1-) + (1-) = 0 </li></ul></ul><ul><ul><li>For every one magnesium ion, we need two chlorine ions </li></ul></ul><ul><ul><li>Chemical Formula </li></ul></ul><ul><ul><li>MgCl 2 </li></ul></ul>
  20. 20. <ul><li>Your turn… </li></ul><ul><li>What is the chemical formula for an ionic compound of </li></ul><ul><li>potassium </li></ul><ul><li>and </li></ul><ul><li>sulfur ? </li></ul>
  21. 21. <ul><li>K 2 S </li></ul><ul><li>Were you correct? </li></ul>
  22. 22. <ul><li>Try some more </li></ul><ul><li>Sodium and Phosphorus </li></ul><ul><li>Lithium and Nitrogen </li></ul><ul><li>Strontium and Bromine </li></ul>
  23. 23. <ul><li>Ask Ms. Acker about the </li></ul><ul><li>Criss - Cross </li></ul>
  24. 24. Goal 3 Name ionic compounds
  25. 25. <ul><li>Step one: </li></ul><ul><ul><li>Say the metal </li></ul></ul><ul><li>Step two: </li></ul><ul><ul><li>Say the nonmetal with an “ ide” ending </li></ul></ul>
  26. 26. <ul><li>NaCl = Sodium Chlor ide </li></ul><ul><li>KCl = Potassium Chlor ide </li></ul><ul><li>MgCl 2 = Magnesium Chlor ide </li></ul><ul><li>KF = _________________ </li></ul><ul><li>Li 2 S = __________________ </li></ul><ul><li>______= Beryllium Sulf ide </li></ul><ul><li>____ = Sodium phosph ide </li></ul>
  27. 27. Goal 4 Use electron dot structures to show ionic compound formation
  28. 28. <ul><li>It’s all about the valence electrons </li></ul><ul><li>Metals give (away extras) </li></ul><ul><li>Nonmetals receive (to fill outer shell) </li></ul><ul><li>Ms. Acker will now show you on the board </li></ul><ul><li>Please take note </li></ul>

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